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Chapter 9: Problem 39

Classify each of the following solids as metallic, network covalent, ionic, or molecular. (a) It is insoluble in water, melts above \(500^{\circ} \mathrm{C}\), and does not conduct electricity either as a solid, dissolved in water, or molten. (b) It dissolves in water but does not conduct electricity as an aqueous solution, as a solid, or when molten. (c) It dissolves in water, melts above \(100^{\circ} \mathrm{C}\), and conducts electricity when present in an aqueous solution.

Short Answer

Expert verified
Question: Based on their properties, classify each of the following solids as metallic, network covalent, ionic, or molecular: (a) Insoluble in water, melts above \(500^{\circ} \mathrm{C}\), does not conduct electricity as a solid, dissolved in water, or molten. (b) Dissolves in water but does not conduct electricity as an aqueous solution, as a solid, or when molten. (c) Dissolves in water, melts above \(100^{\circ} \mathrm{C}\), and conducts electricity when in an aqueous solution. Answer: Solid (a) is a network covalent solid, solid (b) is a molecular solid, and solid (c) is an ionic solid.

Step by step solution

01

(Identify properties of each solid)

Given the properties of each solid, form a basic understanding of the general characteristics of metallic, network covalent, ionic, and molecular solids.
02

(Classify Solid (a))

For solid (a), it is insoluble in water, melts above \(500^{\circ} \mathrm{C}\), and does not conduct electricity either as a solid, dissolved in water, or molten. This solid exhibits characteristics typical of network covalent solids, as they are generally high-melting-point compounds and do not conduct electricity. Therefore, solid (a) is a network covalent solid.
03

(Classify Solid (b))

For solid (b), it dissolves in water but does not conduct electricity as an aqueous solution, as a solid, or when molten. This indicates that the solid is most likely a molecular solid, as these solids often dissolve in water but do not conduct electricity in any state. Therefore, solid (b) is a molecular solid.
04

(Classify Solid (c))

For solid (c), it dissolves in water, melts above \(100^{\circ} \mathrm{C}\), and conducts electricity when present in an aqueous solution. This is a common characteristic of an ionic solid, as they generally dissolve in water and can conduct electricity when in aqueous solutions because the ions are free to move. Therefore, solid (c) is an ionic solid. In conclusion, solid (a) is a network covalent solid, solid (b) is a molecular solid, and solid (c) is an ionic solid.

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